Jespersen 7th Ed. Ch. 0 & 2Activity 2—Periodic Table/NomenclatureCHE 1100R
NAME: ______
Periodic Table
Model 2: Modern Periodic TableIn the Modern Periodic table, the elements are ordered by increasing atomic number. The horizontal row corresponds to filling shells of electrons where the Noble gases at the end of each row correspond to filled shells and are therefore very stable (more about this later).
Periods– horizontal rows in the Periodic Table. For identification purposes they are numbered 1 through 7 starting with the row that only contains H and He.
Groups– vertical columns containing elements with similar properties. They are also referred to as families of elements due to the similarity in properties. There are two numbering conventions are used to label the groups.
- The international scientific convention (IUPAC) numbers each column 1 through 18.
- Chemists in North America favor the system where the longer groups are labeled 1A to 8A (1, 2, 13 – 18 in the IUPAC system) and the shorter groups are labeled 1B to 8B (or 3 – 12 in the IUPAC system) in the sequence depicted in the Periodic Table at the end of this activity.
- A groups are known as the representative or main group elements.
- B groups are called the transition elements. They are located in the center of the periodic table.
- Group numbers 1A through 8A tell you the number of valence electrons an element has.
Inner transition elements– elements in the two long rows below the main body of the table.
- Each row is named after the element that it follows in the main body of the table.
- Elements 58–71 are thelanthanide elements because they follow lanthanum (Z = 57)
- Elements 90–103 are theactinide elements because they follow actinium (Z =89).
- i.e., in groups 3A – 6A that occur in rows 4 – 7 of the periodic table.
- Ex. Tin (Sn) and lead (Pb)
There are three categories of elements in the Periodic Table: metals, nonmetals, and metalloids.
Metals are located in the left and center.
- Good conductors of heat and electricity.
- Readily lose electrons to form positive ions, called cations.
- Poor conductors of heat and electricity.
- Readily gain electrons to form negative ions, called anions.
- Eight elements on a diagonal line: B, Si, Ge, As, Sb, Te, Po and At.
- Also called semimetals or semiconductors because their conductivity is between that of metals nonmetals.
Key Questions:
1.What information about an element is provided in each box for that element in the Periodic Table in the model?
2.What determines the sequence of the elements from the first to the last?
3.Where are the metals, nonmetals, and metalloids located?
4.What is the difference between a group and a period?
5.How can you determine the total number of electrons that a neutral atom has from the Periodic Table?
6.How can you determine the number of valence electrons that atoms in groups 1, 2 and 13 through 18 have?
7.Helium is a monatomic gas, and it extremely unreactive. What other elements would we expect to have similar properties?
Exercises:
1.Write the name, symbol, atomic number, and average mass for the Group 2 metal in Period 3.
2.Write the name, symbol, average mass, and number of protons for the Group 16 nonmetal in Period 2.
3.Write the name, symbol, average mass, and number of electrons for the Group 15 metalloid in Period 4
4.Write the name and symbol of the uncharged element that has 48 electrons.
5.Name two elements that have properties similar to sodium, Na. How many valence electrons does each of these three elements have?
Model 3:Naming Binary Compounds/Nomenclature- Binary compounds are molecules or ionic compounds that are composed of only two elements.
- In general, we name each element in the order they appear in the chemical formula.
- For the first element, we use the English name of the element
- For the second element, we use the stem of the English name and add the ide ending.
Chemical Symbol / Stem / Name as First Element / Name as Second Element
O / ox– / oxygen / oxide
N / nitr– / nitrogen / nitride
P / phosph– / phosphorous / phosphide
S / sulf– / sulfur / sulfide
Cl / chlor– / chlorine / chloride
F / fluor– / fluorine / fluoride
Br / brom– / bromine / bromide
I / iod– / iodine / iodide
Key Questions:
8.What does the term binary covalent mean?
9.What ending is applied to the root of the second element in the name?
Model 3 A:Naming Binary Covalent CompoundsA binary covalent compound is formed from two different non-metals.
In covalentmolecules we use using number prefixes before each element name to indicate the number of each type of element.
1.Number prefix + 1st element English name
2.Number prefix + stem of 2nd second element English name + ide.
Table 3. Greek Number Prefixes
Greek prefixes / Number of like atoms / Greek prefixes / Number of like atoms
mono / 1 (omitted on 1st atom) / hexa / 6
di / 2 / hepta / 7
tri / 3 / octa / 8
tetra / 4 / nona / 9
penta / 5 / deca / 10
Table 4. Examples of Naming Binary Covalent Molecules
Molecular Formula / Name / Molecular Formula / Name
HCl / hydrogen chloride / H2S / hydrogen sulfide
CO / carbon monoxide / PBr3 / phosphorous tribromide
CO2 / carbon dioxide / CCl4 / carbon tetrachloride
There are a few exceptions were we use the common name rather than the name based on the rules above.
H2O is waterNH3 is ammonia
Key Questions:
10.What prefixes are used to indicate the number of atoms when there is more than one possibility?
11.In what types of compounds do you use number prefixes?
Exercises:
6.For each molecular compound given below fill in the missing name or formula.
Molecular Formula / NameSO3
dinitrogen tetrasulfide
PF5
carbon tetrachloride
HBr
tellurium dihydride
N2O5
nitrogen dioxide
Model 3B:Naming Binary Ionic Compounds
Binary ionic compounds consist of a metal and a nonmetal.
The metal forms the cation and the nonmetal is the anion.
Namingioniccompounds:
- The cationis named first using the element’s English name.
- The anion name is named second using the stem of the element’s English name and adding ide to the end.
3.If a metal forms onlyone positiveion, the cation name is the English name for the metal.
4.Transition metals and Post Transition Metals that can have more than one charge:
- Give the English name for the cation followed, without a space, by the numerical value of the charge written as a Roman numeral in parentheses.
Main Group Metals / Common Charges / Main Group Metals / Common Charges
Sodium / Na+ / Alkali Metals / +1
Magnesium / Mg2+ / Alkaline Earth metals / +2
Aluminum / Al3+
Transition Metals / Common Charges / Transition Metals / Common Charges
Chromium / Cr2+, Cr3+ / Copper / Cu+, Cu2+
Manganese / Mn2+, Mn3+ / Zinc / Zn2+
Iron / Fe2+, Fe3+ / Silver / Ag+
Cobalt / Co2+, Co3+ / Cadmium / Cd2+
Gold / Au+, Au3+ / Nickel / Ni2+
Mercury / Hg22+, Hg2+
Post-transition Metals / Common Charges / Post-transition Metals / Common Charges
Tin / Sn2+, Sn4+ / Bismuth / Bi3+
Lead / Pb2+, Pb4+
The Group 5 non-metal anions have a charge of –3, the Group 6 anions have a charge of –2, and the Group 7 anions have a charge of –1.
Writing formulas of ionic compounds from their names:
- The cation is given first in the formula and the anion is given second.
- The subscripts in the formula must produce an electrically neutral chemical formula.
- The subscripts should be a set of the smallest whole numbers possible.
- The charges on ions are not included in the finished formula of the substance.
Molecular Formula / Name / Ionic Formula / Name
NaCl / sodium chloride / CoCl2 / Cobalt(II) chloride
KBr / potassium bromide / CoCl3 / Cobalt(III) chloride
MgCl2 / magnesium chloride / FeO / Iron(II) oxide
CaCl2 / calcium chloride / Fe2O3 / Iron(III) oxide
CaO / calcium oxide / Al2O3 / Aluminum oxide
Key Questions:
12.In the formula and the name, which element is given first, the metal or the nonmetal?
13.What ending is applied to the root of the nonmetal in an ionic compound?
14.When a metal ion can form more than one kind of cation, how is the charge on the cation indicated?
15.Since a Roman numeral is not included in the names of the alkali metal and alkaline earth metal compounds, how do you determine the charge on the cation and the number of anions associated with it?
16.Why do Na and Cl combine to form NaCl instead of Na2Cl?
Exercises:
7.For each ionic compound given below fill in the missing name or formula.
Ionic Formula / NameK2O
Cr2O3
ZnBr2
copper(I) sulfide
calcium fluoride
mercury(II) nitride
9.Which type of compounds contains numeric prefixes? Which type does not?
9.How can you tell from the name if a binary compound is covalent or ionic?
10.For the following compounds, identify the compound as covalent or ionic and complete the table by filling in the missing entries.
Type (ionic or covalent) / Formula / NameCS2
N2O4
sodium sulfide
Cu2O
FeCl3
chromium(III) bromide
Model 3C:Names of Polyatomic Ions
Polyatomic ions
- Ions composed of two or more atoms linked by covalent bonds
- If ions are negative, they have too many electrons
- If ions are positive, they have too few electrons
- Follow same rules as ionic compounds
- Polyatomic ions are expressed in parentheses
- Follow same rules as ionic compounds
- Use names given in table for each polyatomic ion. These common names follow rules you will learn later in your courses. You would be well served to memorize the names of these common ions.
Polyatomic Ion / Name / Polyatomic Ion / Name
NH4+ / ammonium ion / ClO– / hypochlorite ion
H3O+ / hydronium ion / ClO2– / chlorite ion
OH– / hydroxide ion / ClO3– / chlorate ion
CN– / cyanide ion / ClO4– / perchlorate ion
NO2– / nitrite ion / MnO4– / permanganate ion
NO3– / nitrate ion / CO32– / carbonate ion
C2H3O2– / acetate ion / HCO3– / hydrogen carbonate ion (bicarbonate ion)
C2O42– / oxalate ion / SCN– / thiocyanate ion
SO32– / sulfite ion / HSO3– / hydrogen sulfite ion (bisulfite ion)
SO42– / sulfate ion / HSO4– / hydrogen sulfate ion (bisulfate ion)
S2O32– / thiosulfate ion / PO43– / phosphate ion
CrO42– / chromate ion / HPO42– / monohydrogen phosphate ion
Cr2O72– / dichromate ion / H2PO4– / dihydrogen phosphate ion
Key Questions:
17.When two similar polyatomic ions exist with different numbers of oxygen atoms, how do the names distinguish between these?
18.How does the name identify a polyatomic ion as having a positive charge?
19.If a polyatomic ion appears in the name of a compound, what can you deduce about the chemical nature of the compound?
Exercises:
11.For each of the following ionic compounds involving polyatomic ions fill in the missing name or formula.
Ionic Formula / NameCuNO3
manganese(II) acetate
Ca(OH)2
ammonium sulfite
K3PO4
lithium hypochlorite
Fe(SCN)2
aluminum oxalate
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Jespersen 7th Ed. Ch. 0 & 2Activity 2—Periodic Table/NomenclatureCHE 1100R
Periodic Table of the Elements
1 / 2 / 3 / 4 / 5 / 6 / 7 / 8 / 9 / 10 / 11 / 12 / 13 / 14 / 15 / 16 / 17 / 181A / 2A / 3B / 4B / 5B / 6B / 7B / 8B / 8B / 8B / 1B / 2B / 3A / 4A / 5A / 6A / 7A / 8A
1 / 1 / Atomic Number / 2
H / H / Symbol / He
Hydrogen / Hydrogen / Element Name / Helium
1.008 / 1.008 / Mean Atomic Mass (amu)/Molar Mass (g/mol) / 4.002
3 / 4 / 5 / 6 / 7 / 8 / 9 / 10
Li / Be / B / C / N / O / F / Ne
Lithium / Berylium / Boron / Carbon / Nitrogen / Oxygen / Fluorine / Neon
6.941 / 9.012 / 10.81 / 12.01 / 14.01 / 16.00 / 18.99 / 20.18
11 / 12 / 13 / 14 / 15 / 16 / 17 / 18
Na / Mg / Al / Si / P / S / Cl / Ar
Sodium / Magnesium / Aluminum / Silicon / Phosphorus / Sulfur / Chlorine / Argon
23.00 / 24.31 / 26.98 / 28.09 / 30.97 / 32.07 / 35.45 / 39.95
19 / 20 / 21 / 22 / 23 / 24 / 25 / 26 / 27 / 28 / 29 / 30 / 31 / 32 / 33 / 34 / 35 / 36
K / Ca / Sc / Ti / V / Cr / Mn / Fe / Co / Ni / Cu / Zn / Ga / Ge / As / Se / Br / Kr
Potassium / Calcium / Scandium / Titanium / Vanadium / Chromium / Manganese / Iron / Cobalt / Nickel / Copper / Zinc / Gallium / Germanium / Arsenic / Selenium / Bromine / Krypton
39.10 / 40.08 / 44.96 / 47.87 / 50.94 / 52.00 / 54.94 / 55.85 / 58.93 / 58.69 / 63.55 / 65.39 / 69.72 / 72.61 / 74.92 / 78.96 / 79.904 / 83.80
37 / 38 / 39 / 40 / 41 / 42 / 43 / 44 / 45 / 46 / 47 / 48 / 49 / 50 / 51 / 52 / 53 / 54
Rb / Sr / Y / Zr / Nb / Mo / Tc / Ru / Rh / Pd / Ag / Cd / In / Sn / Sb / Te / I / Xe
Rubidium / Strontium / Yttrium / Zirconium / Niobium / Molybdenum / Technetium / Ruthenium / Rhodium / Palladium / Silver / Cadmium / Indium / Tin / Antimony / Tellurium / Iodine / Xenon
85.47 / 87.62 / 88.91 / 91.22 / 92.91 / 95.94 / (98) / 101.07 / 102.91 / 106.42 / 107.87 / 112.41 / 114.82 / 118.71 / 121.76 / 127.60 / 126.04 / 131.29
55 / 56 / 57 / 72 / 73 / 74 / 75 / 76 / 77 / 78 / 79 / 80 / 81 / 82 / 83 / 84 / 85 / 86
Cs / Ba / *La / Hf / Ta / W / Re / Os / Ir / Pt / Au / Hg / Tl / Pb / Bi / Po / At / Rn
Cesium / Barium / Lanthanum / Hafnium / Tantalum / Tungsten / Rhenium / Osmium / Iridium / Platinum / Gold / Mercury / Thallium / Lead / Bismuth / Polonium / Astatine / Radon
132.90 / 137.33 / 138.91 / 178.49 / 180.95 / 183.84 / 186.21 / 190.23 / 192.22 / 195.08 / 196.97 / 200.59 / 204.38 / 207.2 / 208.98 / (209) / (210) / (222)
87 / 88 / 89 / 104 / 105 / 106 / 107 / 108 / 109 / 110 / 111 / 112 / 113 / 114 / 115 / 116 / 117 / 118
Fr / Ra / †Ac / Rf / Db / Sg / Bh / Hs / Mt / Ds / Rg / Cn / Uut / Fl / Uup / Lv / Uus / Uuo
Francium / Radium / Actinium / Rutherdfordium / Dubnium / Seaborgium / Bohrium / Hassium / Meitnerium / Darmstadtium / Roentgenium / Copernicium / Flerovium / Livermorium
(223) / 226.02 / 227.03 / 261.11 / 262.11 / 263.1 / 262.12 / 265.13 / (268) / (269) / (272) / (277) / (284) / (289) / (288) / (293) / (297) / (294)
Alkali metals / Alkaline earth / Transition Metals / Halogens / Noble Gases
metals / *Lanthanides / 58 / 59 / 60 / 61 / 62 / 63 / 64 / 65 / 66 / 67 / 68 / 69 / 70 / 71
/ Ce / Pr / Nd / Pm / Sm / Eu / Gd / Tb / Dy / Ho / Er / Tm / Yb / Lu
Cerium / Praseodymium / Neodymium / Promethium / Samarium / Europium / Gadolinium / Terbium / Dysprosium / Holmium / Erbium / Thulium / Ytterbium / Lutetium
/ 140.12 / 140.91 / 144.24 / (144) / 150.36 / 151.96 / 157.25 / 158.92 / 162.50 / 164.93 / 167.26 / 168.93 / 173.04 / 174.97
†Actinides / 90 / 91 / 92 / 93 / 94 / 95 / 96 / 97 / 98 / 99 / 100 / 101 / 102 / 103
/ Th / Pa / U / Np / Pu / Am / Cm / Bk / Cf / Es / Fm / Md / No / Lr
Thorium / Protactinium / Uranium / Neptunium / Plutonium / Americium / Curium / Berkelium / Californium / Einsteinium / Fermium / Mendelevium / Nobelium / Lawrencium
232.04 / 231.04 / 238.03 / 237.05 / (244) / (243) / (247) / (247) / (251) / (252) / (257) / (258) / (259) / (26O)
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